1. Chemical Names and Formulas In chemistry, chemical names and formulas are used interchangeably. You must learn how to shift back forth between them, if given a name, write a formula, and visa versa. We will start with the simplest inorganic compounds, binary salts.

2. Inorganic Nomenclature Naming Ionic Compounds and Writing Formulas

3. Naming Binary Ionic Compounds Binary ionic compounds consist of a metal cation and a non-metal anion. The metal always comes first. The –ide suffix is added to the end of the non- metal. Sodium chlorideMagnesium oxide Potassium sulfideAluminum bromide

4. Given the formula, write the name 1) MgS 2) KBr 3) Ba 3 N 2 4) Al 2 O 3 5) NaI 6) SrF 2

5. 7) Li 2 S 8) RaCl 2 9) CaO 10) AlP

6. Given the name, write the formula Look up the common ionic charge for the metal and non-metal on your reference table This is shown as “Selected Oxidation States,” in the top right hand corner of each element. Note that non-metals often have more than one oxidation state: ignore all but the top one for now.

7. Magnesium Oxide formula Look up oxidation states of Mg and O Write each as an cation and anionMg 2+ O 2- Criss cross the charges, making them subscriptsMg 2 O 2 Reduce by dividing by common denominator, if necessary MgO

8. Oxidation numbers without lookups

9. Names  Formulas 2) lithium bromide 3) calcium nitride 4) aluminum sulfide 5) potassium iodide 6) strontium chloride

10. 7) sodium sulfide 8) radium bromide 9) magnesium sulfide 10) aluminum nitride 11) cesium sulfide 12) potassium chloride 13) strontium phosphide

11. Polyvalent Metals Many of the d-block metals (transition metals) are polyvalent: they have more than one type of ion. For example, iron: Fe 2+ and Fe 3+ There are two compounds of iron and oxygen: FeO and Fe 2 O 3 Roman numerals are used to indicate the charge on the cation – they become iron (II) oxide and iron (III) oxide, respectively.

12. Common Polyvalent Metals FeCuSn AuHgPb CrMnCo

13. Rules for converting names to formulas Write ionic charges for polyvalent metal next to the symbol, look up oxidation number for the non-metal (always the negative one!) Criss-cross the charges to become subscripts; reduce to lowest common denominator (if necessary).

14. Formulas –> Names 1) iron(II) chloride 2)copper(I) sulfide 3) lead(IV) iodide 4) tin(II) fluoride 5) mercury(I) bromide 6) tin(II) oxide

15. 7) chromium(III) oxide 8) gold(I) iodide 9) manganese(II) nitride 10) cobalt(III) phosphide 11) iron(III) chloride 12) copper(II) sulfide 13)lead(II) bromide

16. Rules for converting formulas to names Look up oxidation number of non-metal (always the negative one!) Count number of negative charges, divide by subscript of the metal Write I, II, III, etc. after the metal name, followed by the anion.

17. Formulas  Names 1) CuS 2) PbBr 4 3) Pb 3 N 2 4) Fe 2 O 3 5) FeI 2 6) Sn 3 P 4

18. 7)Cu 2 S 8)SnCl 2 9)HgO 10)Hg 2 F 2 11)CuCl 2 12)CuBr 13)PbO

19. Polyatomic Ions Many ions are actually made of two or more non-metals. Polyatomic ions have suffixes such as –ite, and –ate that you have heard throughout your lives. Reference Table E lists the more common polyatomic ions.

21. Ternary Ionic Compounds Compounds containing polyatomic ions commonly have three or more different elements These are called ternary ionic compounds. You will need to learn to recognize polyatomic ions in names and formulas, and go to your reference tables to make conversions Memorizing polyatomic names, formulas and charges is a good idea for future science majors

22. Names  Formulas 1)silver carbonate 2) potassium hydrogen phosphate 3) aluminum hydroxide 4) sodium hydrogen carbonate 5) calcium acetate 6) potassium permanaganate 7) calcium perchlorate 8) lithium carbonate

23. Names  Formulas 9) magnesium hydrogen sulfite 10) sodium hypochlorite 11) tin(IV) chlorite 12) mercury(II) phosphate 13) tin(II) carbonate 14) mercury (I) acetate 15) lead(II) chromate 16) copper(I) sulfite 17) Tin (II) dichromate

24. Formulas  Names 1) AlPO 4 2) KNO 2 3)NaHCO 3 4) CaCO 3 5) Mg(OH) 2 6) Na 2 CrO 4

25. 7) Ba(CN) 2 8) K 2 SO 4 9) NaH 2 PO 4 10) NH 4 NO 3 11) Sn(NO 3 ) 2 12) FePO 4 13) Cu 2 SO 4 14) Ni(C 2 H 3 O 2 ) 2 15) HgCO 3

26. All Types Together!! NaMnO 4 PbSO 4 AlBr 3 NH 4 NO 3 FePO 4 Al 2 (SO 4 ) 3 KCN

27. KHCO 3 Hg(OH) 2 Sn(HCO 3 ) 4 NaH Fe(ClO 4 ) 3 Cu 2 CrO 4

28. Iron (II) hydrogen sulfite Aluminum perchlorate Calcium chlorate Ammonium hydroxide Cobalt (II) iodide Iron (III) carbonate Iron (II) oxide Silver sulfide

29. Potassium nitrate Potassium nitrite Ammonium chromate Lead (IV) chlorite Silver oxide Iron (III) hydrogen carbonate Barium hypochlorite Copper (I) carbonate

30. Chemical NameChemical Formula Metals are always stated first, by using the name of the element.Metals first, non-metals second. Subscripts indicate the number of atoms of each element in the compounds. Non-metals are stated second. They always end with an –ide suffix (sodium choride) Parenthesis (often used for polyatomic ions) indicate that everything inside must be multiplied by the subscript. Ex: Ca(NO 3 ) 2 has 2 atoms of N and 6 of O. Metals with more than one valence are called polyvalent metals. The charge on the ion (always positive) can be found on the periodic table in the upper right corner of each element (oxidation numbers) Polyvalent metals must be recognized! The common ones are Fe, Co, Au, Pb, Sn, Cu, Mn, Cr, and Hg. The charge on the metal can be determined from the non-metal or polyatomic ion. Polyvalent metals are given Roman numerals to distinguish them from each other. (ex: Iron (II) and Iron (III)) Count the total number of negative charges (the charge on the ion * subscript on the ion) and divide by the number of atoms of the cation to get the charge on the cation. Polyatomic ions are made up of combinations of non-metals, and occasionally metals. The charges on the polyatomic ions are found on Table E. Polyatomic ions have unique names and charges. Many of them end in – ate or –ite suffixes. Most are negative ions. They can be found on Table E (front page) Polyatomic ions always have the same charge. Chemical names often must be converted into formulas. Here is a simple way to do this: 1.Write the name of the metal, followed by the non-metal or polyatomic ion. 2.Write the charge of the negative ion as a superscript to the right of the symbol. For non-metals, the charge is always the top oxidation number on the periodic table. Polyatomic charges must be looked up on Table E. 3.Write the charge on the positive ion, given in the periodic table or in the chemical name 4.Criss-cross the ionic charges; the anion supersript becomes the cation subscript; the cation charge becomes the number of anions. 5.If necessary, reduce to lowest common denominator. Examples: CaCl 2 1.chloride has –1 charge. Calcium is always +2. 2.Write name: calcium chloride (no II necessary) Fe(NO 3 ) 3 1.NO 3 is nitrate (Table E), w/ -1 charge 2.Fe can be II or III. Which one? 3.Since there are 3 nitrates, the charge on the Fe must be +3 4.Write the name: iron (III) nitrate. Ex. Barium Sulfate: Ba is +2; sulfate is SO 4 2- from table E. Criss cross leaves Ba 2 (SO 4 ) 2 Reduce to lowest common denomentator: BaSO 4. (NH 4 ) 2 CO 3 : Both of these ions are on Table E! NH 4 + is ammonium; CO 3 2- is carbonate; ammonium carbonate